Sodium iodate

Sodium iodate
Other names iodic acid, sodium salt
Identifiers
CAS number	7681-55-2 N
PubChem	23675764
ChemSpider	22760 Y
RTECS number	NN1400000
Jmol-3D images	{{#if:[Na+].[O-]I(=O)=O|Image 1
SMILES [Na+].[O-]I(=O)=O
InChI InChI=1S/HIO3.Na/c2-1(3)4;/h(H,2,3,4);/q;+1/p-1 Y Key: WTCBONOLBHEDIL-UHFFFAOYSA-M Y InChI=1/HIO3.Na/c2-1(3)4;/h(H,2,3,4);/q;+1/p-1 Key: WTCBONOLBHEDIL-REWHXWOFAB
Properties
Molecular formula	NaIO3
Molar mass	197.8924 g/mol
Appearance	white orthorhombic crystals
Density	4.28 g/cm³, solid
Melting point	425 °C (decomp) [1] (anhydrous) 19.85 °C (pentahydrate)
Solubility in water	9.47 g/100 mL (25 °C) 34 g/100 mL (100 °C)
Solubility	soluble in acetic acid insoluble in alcohol
Hazards
EU classification	not listed
NFPA 704	1 1 OX
Related compounds
Other anions	sodium iodide sodium periodate sodium bromate sodium chlorate
Other cations	potassium iodate silver iodate
N (verify) (what is: Y/N?) Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
Infobox references

Sodium iodate (NaIO₃) is the sodium salt of iodic acid. Sodium iodate is an oxidizing agent, and as such it can cause fires upon contact with combustible materials or reducing agents.

Preparation

It can be prepared by reacting a sodium-containing base such as sodium hydroxide with iodic acid, for example:

HIO₃ + NaOH → NaIO₃ + H₂O

It can also be prepared by adding iodine to a hot, concentrated solution of sodium hydroxide or its carbonate:

3 I₂ + 6 NaOH → NaIO₃ + 5 NaI + 3 H₂O

Reactions

Sodium iodate can be oxidized to sodium periodate in water solutions by hypochlorites or other strong oxidizing agents:

NaIO₃ + NaOCl → NaIO₄ + NaCl

Safety

Conditions/substances to avoid are: heat, shock, friction, combustible materials, reducing materials, aluminium, organic compounds, carbon, hydrogen peroxide, sulfides.

References